×
Log in to StudySoup
Get Full Access to Chemistry - Textbook Survival Guide
Join StudySoup for FREE
Get Full Access to Chemistry - Textbook Survival Guide

A 10.0-mL sample of a commercial hydrogen peroxide (H2O2)

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 101P Chapter 16

Introductory Chemistry | 5th Edition

  • Textbook Solutions
  • 2901 Step-by-step solutions solved by professors and subject experts
  • Get 24/7 help from StudySoup virtual teaching assistants
Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

4 5 1 402 Reviews
23
5
Problem 101P

A 10.0-mL sample of a commercial hydrogen peroxide (H2O2) solution is titrated with 0.0998 M KMnO4. The end point is reached at a volume of 34.81 mL. Find the mass percent of H2O2 in the commercial hydrogen peroxide solution. (Assume a density of 1.00 g/mL for the hydrogen peroxide solution.) The unbalanced redox reaction that occurs in acidic solution during the titration is:

H2O2(aq) + MnO4− (aq) → O2(g) + Mn2+ (aq)

Step-by-Step Solution:

Here we have to calculate the mass percent of H2O2 in sample.

Step 1:

The balanced equation for the redox reaction is

2 MnO−4 (aq) + 5H2O2 (aq) + 6 H+(aq) → 2 Mn2+(aq) + 5 O2(g) + 8 H2O(l)

Step-3

Molar mass of H2O2 = 34.014 g/mol

Mass percent = (grams of solute / grams of solute plus solvent)  100

Volume of H2O2 = 10.0 mL

Density of H2O2 = 1.00 g/mL

It is known that d = m/V

m = d  V

    = 1.00 g/mL10.0mL = 10 g (mass of H2O2)

Concentration of KMnO4 = 0.0998 M

Final volume = 34.81 mL= 0.3481 L

C = moles / liters

Or, C = (grams / Molar mass) / (liters)

Or, C = (m / M ) / V = m / (M V)

m = CMV

    = 0.998 158.034...

Step 2 of 3

Chapter 16, Problem 101P is Solved
Step 3 of 3

Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. The full step-by-step solution to problem: 101P from chapter: 16 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. Since the solution to 101P from 16 chapter was answered, more than 398 students have viewed the full step-by-step answer. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. This full solution covers the following key subjects: solution, hydrogen, peroxide, commercial, occurs. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The answer to “A 10.0-mL sample of a commercial hydrogen peroxide (H2O2) solution is titrated with 0.0998 M KMnO4. The end point is reached at a volume of 34.81 mL. Find the mass percent of H2O2 in the commercial hydrogen peroxide solution. (Assume a density of 1.00 g/mL for the hydrogen peroxide solution.) The unbalanced redox reaction that occurs in acidic solution during the titration is:H2O2(aq) + MnO4? (aq) ? O2(g) + Mn2+ (aq)” is broken down into a number of easy to follow steps, and 71 words.

Unlock Textbook Solution

Enter your email below to unlock your verified solution to:

A 10.0-mL sample of a commercial hydrogen peroxide (H2O2)

×
Log in to StudySoup
Get Full Access to Chemistry - Textbook Survival Guide
Join StudySoup for FREE
Get Full Access to Chemistry - Textbook Survival Guide
×
Reset your password